is BrCl5 polar, need help?
"Can someone help me determine if bromine pentachloride (BrCl5) is a polar molecule? I’d appreciate an explanation of the molecular geometry and how it influences the polarity. Thank you!"
5 Answers
BrCl5 has octahedral geometry with square pyramidal shape. BrCl5 has 6 effective pairs around the central Br atom, 5 of which are Br-Cl bonds, while 1 is a lone pair. Since all 6 aren't the same and because the bond dipoles don't all cancel each other out, BrCl5 must be polar.
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To determine the most polar molecule, you first look at the shape of the molecule. CF4 would be a tetrahedral molecule because Carbon has no pairs of lone electrons. BrCl5 would be a trigonal bipyramid because Bromine has no pairs of lone electrons. PCl5 would be a trigonal bipyramid because Phosphorous has no pairs of lone electrons. SCl6 would be a square bipyramid because Sulfur has no pairs of lone electrons. XeF2 would be a linear molecule with lone pairs of electrons on either side of Xenon. Because none of these are polar based on the shape, we now look at the size of the molecules. London Dispersion Forces are the strongest in the largest molecules. LD forces can determine polarity. I would have to say that the largest molecule of this group is BrCl5. ANSWER: BrCl5
the diffrence in electronegativities of Cl and Br is 3.0-2.8=0.2 so it is a non-polar molecule
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